Answer:
Rate of reaction when concentration of A is doubled=0.018 M/s.
Step-by-step explanation:
We are given that for the multi-step reaction
It is given that the rate-limiting step is unimolecular with A as the sole reactant
It means rate of reaction depend upon the concentration of reactant A only
Rate of reaction =k[A]
[A]=0.110 M
[B]=0.110 M
Rate of reaction =0.0090 M/s
According to rate law
Rate of reaction=k[A]
If concentration of A is doubled then the rate of reaction is given by
Rate of reaction =k[2A]= 2 k[A]=2 initial rate of reaction
Therefore, rate of reaction after substituting values
Rate of reaction ==0.018 M/s
Rate of reaction when concentration of A is doubled=0.018 M/s.
Answer: 2,749.50
Step-by-step explanation:
56,715*10.70% = 6068.505
8818 - 6068.505 = 2,749.50
Answer:
(k+3)(k+4)
The zeros are -3 and -4
Step-by-step explanation:
k2+7k+12
The middle number is 7 and the last number is 12.
This means we need two numbers that:
Add together to get 7
Multiply together to get 12
to fit in this equation (k+_)(k+_)
in this equation, it would be 3 and 4
3+4 = 7
3*4 = 12
Now we fill in the blanks to get
(k+3)(k+4)
To get the zeros, use the equations
k+3=0 and k+4=0
You end up with
k=-3 and k=-4
Answer:
Step-by-step explanation:
To add or subtract square roots, you must be taking the square roots of the same number. We need to change square root of 8 into a number times square root of 2.
Now that we have two square roots of 2, we add them like we add like terms.
Answer:look closely
Step-by-step explanation: